Given the following half reaction: a. lt b. Pt| Fe,Fe+3 c. ZnZn 2 d. Ag | Ag For each of the following cell combination and or conditions (where the negative electrode is at the left of the combination). Combination A: a and b Combination B: c measured against a saturated calomel electrode at 30°C Combination C: b and d Combination D: c and a if [H] = 1.20M and [Zn+2] = 0.80M at 25°C Determine anode half reaction, cathode half reaction, overall reaction, cell notation, cell potential, free energy change, spontaneity and the equilibrium constant. The equilibrium constant is related to the standard cell potential through: RT 20 In K nF

Given the following half reaction: a. lt b. Pt| Fe,Fe+3 c. ZnZn 2 d. Ag | Ag For each of the following cell combination and or conditions (where the negative electrode is at the left of the combination). Combination A: a and b Combination B: c measured against a saturated calomel electrode at 30°C Combination C: b and d Combination D: c and a if [H] = 1.20M and [Zn+2] = 0.80M at 25°C Determine anode half reaction, cathode half reaction, overall reaction, cell notation, cell potential, free energy change, spontaneity and the equilibrium constant. The equilibrium constant is related to the standard cell potential through: RT 20 In K nF

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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a. Write the overall cell reaction.
Enter electrons as e". Use smallest possible integer coefficients. If a box is not needed, leave it blank. A voltaic cell is constructed from a standard Pb2+|Pb half cell (E°,red :-0.126V) and a standard Zn2+|Zn half cell (E° red -0.763V). The anode reaction is: + + The cathode reaction is: + + The spontaneous cell reaction is: + + The cell voltage is V.
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Enter electrons as e¯. Use smallest possible integer coefficients. If a box is not needed, leave it blank. A voltaic cell is constructed from a standard Co²+ | Co half cell (E° red = -0.280V) and a standard Mg2+ | Mg half cell (E°red = -2.370V). The anode reaction is: + The cathode reaction is: → + The spontaneous cell reaction is: + The cell voltage is V. ↑ +
In the Zn/Zn²+ cell from the previous question, [Zn²+] at the anode is 1.7 x 10-8 M and the [Zn²+] at the cathode is 5.1 M. What is the value of Ecell (in V) when the concentration cell operates at 25°C? (2 sf) Type your answer...
The value of Ksp for AgBr is 5.4 x 10-13. For the Ag/AgBr electrode, AgBr(s) + e Ag(s) + Br (aq) E°AgBr = +0.070V What will be the potential of a cell constructed of a standard hydrogen electrode as one half-cell and a silver wire coated with AgBr dipping into 0.11 M HBr as the other half-cell? Ecell = V
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Answer the following questions given the cell notation (refer to the Standard Aqueous Reduction Potentials in Aqueous Solution at 25ºC and Standard Reduction Potential for Selected Half-Cells for the E0 values): Fe/Fe^2+ (0.100M) // Cd^2+ (0.001)/Cd a. Jot down the cell reaction b. Calculate Ecell, the polarity of the electrodes and direction of the spontaneous rxn. c. Solve for the Keq